Dehydrochlorination process



United States Patent DEHYDROCHLORINATION PROCESS Franklin Conrad, Baton Rouge, La., assignor to Ethyl Corporation, New York, N. Y., a corporation of Delaware No Drawing. Application April 5, 1955, Serial No. 499,531

11 Claims. (Cl. 260-656) example, is manufactured commercially by two processes:

(l) the hydrochlorination of acetylene and (2) dehydrochlorination of 1,2-dichlorocthane, formed by the chlorination of ethylene. Both of these raw materials, i. e. ethylene and acetylene, are relatively expensive. The chlorination of ethane provides a potentially cheaper route to vinyl chloride since ethane is a much cheaper raw material than those heretofore employed. This chlorination process, however, results in a mixture of dichlorides containing about 90 percent of the relatively inert 1,1-dichloroethane and only about percent of the presently useful 1,2-dichloroethane. As no commercial method has been available for the conversion of 1,1- dichloroethane to vinyl chloride, the chlorination of ethane route to vinyl chloride could not and has not been used to date. Similar considerations apply to the commercial production of vinylidene chloride.

The conventional method for dehydrochlorination of 1,2-dichloroethane involves a thermal process conducted at temperatures ranging between 500 and 600 C. While catalytic processes are known, the degree of improvement in either conversion or reduction of reaction temperature is not sufficient to warrant complication of existing processes. In contrast to its isomer, 1,1-dichloroethane requires unduly high temperatures to thermally produce vinyl chloride. Such temperatures are excessively high for commercial use with known materials of construction, and in addition, the feed material is excessively degraded to carbonaceous tars. havior of these isomeric materials under thermal conditions, it would not be expected that catalysts for 1,2-

dichloroethane dehydrochlorination would appreciably reduce the necessary dehydrochlorination temperature of l,l-dichloroethane, or that such catalysts as have been disclosed (Ghose et al., Petroleum 14, 261 (1951)) would even proportionally reduce the necessary temperature, relative to its effectiveness with the 1,2-isomer.

In addition to requiring high temperatures for dehydrochlorination of the polychloroethanes, a considerable quantity of chloroprene is always formed in prior processes using either 1,1- or l,2 dichloroethane., The presence of chloroprene in the product tends to inhibit subse quent polymerization of the vinyl chloride. This chloroprene problem is particularly acute in the thermal de hydrochlorination of 1,l-dichloroethane since the 1,1- dichloroethane and chloroprene have very similar boiling From a consideration of the be- 1 points and cannot be conveniently fractionated or otherwise separated. Thus, if only a part of the 1,1-d1chloroperatures, and a recycle of unreacted materials is employed, the undesired chloroprene tends to unduly build up in the reactor.

It is accordingly an object of the present invention to provide an improved process for producing chloroethylcues from chloroethanes, and particularly vinyl chloride and vinylidene chloride from ethane. Another object is to provide a process suitable for the dehydrochlorination of 1,1-dichloroethane and 1,1,1-trich1oroethane at relatively low temperatures. Still another object is to provide a process of the above type which forms little or no chloroprene as an impurity. Still another object is to provide a catalytic process for the dehydrochlorination of 1,1-dichloroethane in which the catalyst has a long catalyst life.

pended claims.

We have now found that 1,1-dichloroethane and 1,1,1-

trichloroethane can be economically and efficiently dehydrochlorinated to produce vinyl chloride and vinylidene out at relatively low temperatures. The present dehydro chlorination process for the manufacture of chloroethylenes comprises contacting a polychloroethane of the class consisting of 1,l-dichloroethane and 1,1,l-trichloroethane at a temperature between about 150 and 500 C., preferably below about 320 C., with a dehydrochlorination catalyst selected from the group consisting of metal salts group II of the periodic and metal oxides of a metal in table.

The effectiveness of the dehydrochlorination catalysts employed in the present invention in effecting a substantial reduction in the dehydrochlorination temperature of these polychloroethanes, i. e. reduction of up to 350 C.,

is particularly surprising since these catalysts are known to be relatively inactive in the dehydrochlorination of 1,2-

dichloroethane. At the same time the 1,1-dichloroethane' v is known to be considerably more inert than the 1,2-didehydrochlorinate the 1,1-dichloroethane chloroethane isomer against dehydrochlorination under thermal conditions. It is surprising then, that the present catalyst can be employed at temperatures below about 400 C., preferably below about 320 C., to selectively in the presence of the 1,2-dichloroethane.

The selective nature of this catalytic process is of great economic importance since 1,2-dichloroethane has many valuable uses not shared by its isomer and their separaa difiicult and costlyoperation.

useful means for effecting such a separation. The efiectiveness of the claimed catalyst is also particularly surprising in that it materially reduces or eliminates the. formation of undesired chloroprene.

prior thermal processes result in the formation of over. a. hundred times as much chloroprene as is formed when using the present catalytic process- The above discovery that LI-dichloroethane can eiiiciently and economically dehydrochlorinated to vinyl chloride now provides for the first time an economical route to vinyl chloride from a cheap raw material such as ethane. Thus, ethane can be chlorinated, i. e. either thermally or photochemically, to produce an isomeric mixture of dichloroethanes predominating in the l,l-dichloro-- Other objects and advantages of this invention will become apparent from the following description and ap-,

In general, the p natively, the ethyl chloride can also be produced in the ethane chlorination step along with the dichloroethanes and recovered as a valuable coproduct. When desired, a part of the ethyl chloride so formed can be returned to the chlorination reaction zone for conversion to more dichloroethanes thereby providing a means for controlling the ratio of ethyl chloride to vinyl chloride obtained as products from the combined process.

Catalysts which are suitable for use in the process of the present invention comprise the salts and oxides of the metals of group II of the periodic table, including all of the metals in group IIA and H8. The preferred catalysts are the inorganic salts of the metals of this group. Especially preferred in this class are the halides and oxides of metals in group H of the periodic table selected from the group consisting of magnesium, calcium, strontium, barium, zinc, cadmium and mercury. Other salts of the metals of this group such as the sulfates, nitrates, phosphates, cyanides, acetates, oxalates, propionates and the like are also suitable for use as catalysts in the present invention. Some specific examples of such compounds which can be used alone or in mixture of two ormore thereof are beryllium bromide, beryllium chloride, beryllium fluoride, beryllium oxide, beryllium sulfate, magnesium chloride, magnesium bromide, magnesium iodide, magnesium oxide, magnesium sulfate, magnesium nitrate, magnesium pyrophosphate, magnesium acetate, calcium chloride, calcium bromide, calcium iodide, calcium fluoride, calcium sulfate, calcium cyanide, calcium acetate, calcium oxalate, calcium phosphate, strontium bromide, strontium chloride, strontium iodide, strontium oxide, strontium sulfate, strontium nitrate, strontium oxalate, barium chloride, barium iodide, barium oxide, barium bromide, barium fluoride, barium sulfate, barium nitrate, barium phosphate, barium acetate, radium bromide, radium chloride, zinc bromide, zinc chloride, zinc fluoride, zinc oxide, zinc sulfate, zinc tribasic phosphate, zinc acetate, zinc cyanide, cadmium bromide, cadmium chloride, cadmium iodide, cadmium sulfate, cadmium nitrate, cadmium acetate, mercuric bromide, mercuric chloride, mer

curic sulfate, mercurous bromide, and mercurous iodide. Also suitable as catalysts for this process are those compounds which are converted into halides and/or oxides of the metals described above, under the reaction conditions employed. When employing a halogen salt, it is generally preferable to employ the chlorides of the above metals since they are usually the most economical and most readily obtainable of the halogen salts.

The catalyst can be used as such or can be admixed with or deposited upon a suitable carrier such as pumice, silica, silica gel, asbestos, charcoal, fullers earth, activated alumina, magnesia, silica alumina, diatomaceous earths and the like. Particularly preferred catalysts comprise finely divided activated alumina impregnated with a metal halide selected from the group consisting of magnesium chloride, calcium chloride, zinc chloride and cadmium chloride. When using the carrier material, the active catalyst component generally comprises about 0.1 to 30 percent by weight of the catalytic mixture employed.

In practice, the process of the present invention comprises contacting 1,1-dichloroethane or 1,1,1-trichloroethane or mixtures thereof with the above described catalyst at a temperature between about 150 and 500 C. The dehydrochlorination proceeds smoothly and rapidly so as to convert a considerable amount, frequently up to about 100% percent, of the polychloroethane to the desired chloroethylene. The product mixture is'withdrawn from the reaction zone and passed directly to a condenser to recover the condensable materials while allowing the hydrogen chloride to pass overhead to a recovery system.

Alternatively, the product gases from the reaction zonecan be passed through a hydrogen chloride recovery systion.

tem prior to condensing the higher boiling chloroethylenes and unreacted feed stock. If desired, unreacted 1,1-dichloroethane or 1,1,l-trichloroethane can be recycled to the reaction zone in order to obtain a more complete conversion of feed material to the desired product,

The reaction can be conducted in a wide variety of reaction vessels and can be a continuous or batch opera- The preferred operation involves a continuous vapor phase reaction using a packed or fluidized reactor. In the latter cases, the above described catalyst is preferably deposited on a carrier as hereinbefore described and employed as a lump, pelleted, granular or finely divided material. When it is desired to use a packed bed type of reactor, this catalyst material will usually be present in the form of particles of a size small enough to provide large surface areas for maximum contact with the reactant gases. For use in this type of reactor, it has been found that a particle size of from about 3 to 12 mesh size is very satisfactory; 6 to 10 mesh being a preferred size. In one embodiment of the present invention, the catalyst bed can be of the fluid bed type so as to provide the most eflicient contact between the catalyst and the reactants. While the particle size is not especially critical in this type of operation, it is important and it is normal to employ a fluidizing media having an average particle size between about 50 to 250 mesh and preferably between about 70 and 200 mesh. Particles much less than 250 mesh are sometimes suitable for a fluidized bed reaction but such particles tend to be entrained with the product vapors, whereas particles having a diameter above 50 mesh'result in mechanical difiiculties in the fluidized technique. The catalyst can be fluidized by the passage of the gaseous reactant therethrough at a superficial linear velocity of about 0.1 to 50 feet per second, the actual range depending on whether a stationary or transport bed is employed. For a stationary fluid bed system it is generally preferred to employ a superficial linear velocity of about 0.3 to 3 feet per second, while velocities of about 4 to 10 feet per second are preferred for transport or moving bed systems.

. The fluidized bed can be of a conventional type employing any suitable fluidizing means and can utilize any dc sired temperature controlling means, either internal or external. When desired, however, the catalyst can be removed from the reaction zone and easily regenerated by techniques well known to those skilled in the art.

' In general, it is suitable to use pure 1,1-dichloroethane or 1,l,1-trichloroethane as the feed material in the process so as to obtain maximum benefits of the present invention. However, when desired, it is sometimes preferred to employ a feed stream having other alkanes or chlorinated alkanes therein, such for example as l,2dichloro ethane. In the latter case, it has been found that this component does not react during the concomitant dehydrochlorination of the 1,1-dichleroethane or 1,1,1-trichloroethanc at temperatures below about 400 In general, the reaction rate is dependent upon and increases with an increase in the temperature. employed. In the present process, suitable reaction rates are obtained at temperatures as low' as about C. Generally temperatures between about 150 and 500 C, and preferably between about 250 and 320 C. are employed in the process. Temperatures below 150 C. tend to give uneconomically low conversions. Temperatures above about 500 C. can be used but are generally uneconomical since they frequently result in excessive degradation of the reactants and products to form carbonaceous deposits. Higher temperatures also lead to excessively high corrosion rates of those materials of which the reactor equipment is normally constructed. Moreover, when it is desired to preferentially dehydrochlorinate 1,1-dichloroethane or 1,1,1-trichloroethane in the co-presence of 1,2-dichloroethane, the process can be conducted at a temperature between about 150 and 400 0., preferably between about 250 and 320 C. i

A wide range of pressures are suitable for this invention. While atmospheric pressure operation is suitable in many cases, it is generally preferred to operate at superatmospheric pressure for more efficient conversions to the desired products and more economical recovery of these products from the reaction zone. In practice, pressures in the range of about 1 to 20 atmospheres are preferred, although higher pressures can be used with less satisfactory results.

The reaction or contact time is important. When conducting the process in the vapor phase, the linear velocity of the gaseous material passing through the reaction zone can be controlled to obtain the necessary contact time between reactant and catalyst to promote the desired dehydrochlorination reaction. In general, the most advantageous contact period is dependent upon several variables, such as the scale of the operation, quantity of catalyst in the reactor and the type of reactor employed. For most reactors, it has been found that a contact time of as high as about 25 seconds and as low as about 0.5 second is suitable for the present process. With a contact time below about 0.5 second, the product frequently contains considerable quantities of unreacted feed material. Above about 25 seconds, the impurities tend to increase and the product becomes more difficult to recover in a pure form. For optimum production of a high quality product, however, it is generally preferred to employ a contact period of not more than about 10 seconds.

Various process equipment are suitable for use with the present invention. These can be constructed of any of a large number of common and inexpensive materials. This is in contrast to prior processes requiring costly alloys for high temperature operation. Thus, this process can be conducted in iron or ferrous metal reactors without excessive corosion of the reactor walls.

The following examples describe typical embodiments of this process and are given to illustrate the invention in more detail. All quantities in these examples are given in parts by weight.

EXAMPLE I This example illustrates the benefits obtained by the present invention when the process is conducted in a fixed or packed bed type of reactor. The catalysts employed in the following runs were prepared by mixing a solution of 15 parts of the metallic catalyst, e. g. CaClz, MgCl2, BaClz, ZnClz, CdClz, ZnO, MgBrz, BeFz, in 200 parts of water with 300 parts of a diatomaceous earth, i. e. cellite (8-l2 mesh) and drying the mixture in a vacuum oven for 9 hours. The dried material was then ground in a ball-mill and screened to obtain particles between 6 to 10 mesh in size.

A liquid 1,1-dichloroethane feed stream is fed to a vaporizer and the resultant vapors are then passed through a heated reactor tube packed with the catalyst material prepared as described above. The feed rate is regulated so as to permit a contact time of about 2.5 seconds at a reaction temperature of about 300 C. The conversions of 1,1-dichloroethane to vinyl chloride are above 65 percent.

When 1,1,l-trichloroethane is employed in the place of 1,1-dichloroethane in this example, the conversions to vinylidene chloride are above 90 percent.

In a comparative series of runs in which the feed material is 1,2-dichlorocthane, conditions being otherwise the same as above, essentially no reaction is obtained, all of the feed material being recovered in an unreacted form.

EXAMPLE II This comparative example demonstrates the relative difliculty of dehydrochlorinating l,l-dichloroethane in the absence of catalysts of the present invention. Thus, at temperatures as high as 500 C. and in the absence of any catalyst, 1,2-dichloroethane has a dehydrochlorination rate about times as fast as the 1,1-dichloroethane.

Table I Reactor Temperature Conversion to CzHsCI (percent) Catalyst Feed Material None 1,1-dichloroethane.- N one 1,2-dlchloroethane.

It should be noted that even at much higher temperatures, i. e. 500 C., the catalytic dehydrochlorination rate of the 1,1-dichloroethane is less than 5 the rate obtained in Example I.

EXAMPLE III This example illustrates the method of advantageously conducting the present invention in a stationary fluidized bed type reactor. The same feed system and recovery system employed in the process of Examples I and II were used in this example. The catalyst was prepared as in Example I except that the carrier was activated alumina and the mixture was ground so as to obtain a particle size distribution between about 70 and 200 mesh, with an average particle size of about mesh. This catalyst material was packed into the reactor tube so as to occupy approximately one-half of the void space when at rest. The finely divided particles were maintained in a fluidized state by the flow of the reactant gases through the reaction zone. Liquid 1,1-dichloroethane was vaporized and the vapors passed through the fluidized bed reaction zone at a rate of 5.4 moles per hour and at a superficial linear velocity of about 1 foot per second based on the empty reactor.

In a comparative run, 1,2-dichloroethane was employed as a feed material instead of 1,1-dichloroethane. The comparative results are shown in Table II.

Table II Reactor Temper- Trme ature (sec.) 0.) (percent) Contact Catalyst Feed Material Bach {l,1-dichloroethane CaClz 1,1-dichloroethane. M Clz {lg-gicgoroeglfianehfl. 1,1- ic oroe ane Cdclz ilzgicfioroetlhanmflu 1,1- to oroet ane Z1101? {1,2-dichloroethane The results given in Table II show the excellent conversions of 1,1-dichloroethane to vinyl chloride when subjected to the low reaction temperatures and short contact times of the process of the present invention. It should also be noted that when 1,2-dichloroethane was employed as the feed material no appreciable dehydrochlorination was obtained even at 3 times the contact period employed for the 1,1-dichloroethane.

EXAMPLE IV This example contrasts the tremendous reduction in the formation of chloroprene during the dehydrochloiination of 1,1-dichloroethane in the process of this invention with prior thermal processes and the results obtained are given in Table III below. The apparatus and procedures employed in the runs shown in Table III were similar to those of Example III.

As noted in these results, even at lower conversion levels, the thermal non-catalytic process produces over a hundred times as much chloroprene as the catalytic process of this invention. The reduction in chloroprene formation is extremely important in those process operations wherein only a part of the dichloroethane is dehydrochlorinated per pass thereby necessitating the recycle of unreacted reactants in order to obtain a more complete utilization of the raw materials. Since it is extremely difficult to separate the l,l=dichloroethane from any co-present chloroprene due to their close physical and chemical properties, the chloroprene builds up to an untenable concentration after only a few passes. In the present process, however, the low chloroprene formation eliminates the problem. Moreover, if desired, it is now possible to obtain essentially 100 percent conversion of the dichloroethane in the present invention with essentially no chloroprene formation as well as eliminating the need of any recycle operation.

EXAMPLE V The runs in this example Were conducted to demonstrate the long catalyst life exhibited by the catalysts employed in the present invention. The procedures and catalysts employed were the same as in Example III and the results obtained over a 3-hour period showed a continuing high level of conversion of 1,1-dichloroethane to vinyl chloride.

EXAMPLE VI In this example the runs of Example III are repeated except that 1,1,1-trichloroethane is employed as the polychloroethane. Under similar procedures and reaction conditions as used in Example III, the conversion to vinylidene chloride is above 90 percent.

EXAMPLE VII In this example the runs of Example III are repeated except that the catalysts deposited on the activated alumina carrier are beryllium chloride, magnesium fluoride, strontium chloride, mercuric chloride, calcium oxide, cadmium oxide and barium iodide. The reaction conditions are the same as those employed in Example III and the conversions of 1,1-dichloroethane to vinyl chloride are above 60 percent in all the runs.

EXAMPLE VIII The procedures of Example III are repeated in this example except that the catalysts deposited on the activated alumina carrier are magnesium sulfate, magnesium acetate, calcium sulfate, calcium pyrophosphate, calcium oxalate, barium nitrate, barium acetate, zinc sulfate, zinc cyanide and cadmium sulfate. Under the same reaction conditions as employed in Example III the conversions of 1,1-dichloroethane to vinyl chloride are above 50 percent in all of the runs.

Similarly, equally good results are also obtained when using other catalysts of the present invention such as beryllium bromide, beryllium sulfate, cadmium fluoride, cadmium nitrate, cadmium acetate, calcium cyanide, calcium nitrate, calcium fluoride, zinc bromide, zinc iodide, zinc acetate, calcium oxide, calcium bromide, mercuric bromide, mercuric iodide, mercuric sulfate strontium bromide, strontium iodide, barium bromide and barium fluoride and barium sulfate in the illustrative examples given above.

Reaction temperatures as low as C. and as high as 500 C. when employed in similar examples produce essentially comparable results.

As is apparent from the above, the present invention provides an improved process for the economical dehydrochlorination of a cheap raw material, i. e. 1,1-dichloroethane and 1,1,1-trichloroethane, to a valuable product, i. e. the corresponding chloroethylenes. The process also provides a novel and economical route to the manufacture of vinyl chloride from ethane which includes a chlorination and catalytic dehydrochlorination operation. The present process involves the use of a selective catalyst for dehydrochlorinating these polychloroethanes at a temperature between about 15 0 and 500 C. The selective nature of the catalyst is further emphasized by the ability to selectively dehydrochlorinate 1,1-dichloroethane in the presence of its isomer, 1,2-dichloroethane thereby permitting the recovery of a relatively pure co-product which is particularly valuable as a scavenger in motor fuels.

I claim:

1. A process for the manufacture of chloroethylenes which comprises contacting a polychloroethane of the class consisting of 1,1-dichloroethane and 1,1,l-trichloroethane at a temperature between about 150 and 500 C. with a catalyst selected from the group consisting of metal salts and metal oxides, said metal being in group II of the periodic table.

2. The process of claim 1 wherein the metal salts are metal halides.

3. The process of claim 1 in which the catalyst is supported on a carrier.

4. The process of claim 1 wherein the catalyst is magnesium chloride and the carrier is activated alumina.

5. The process of claim 1 wherein the catalyst is cadmium chloride and the carrier is activated alumina.

6. In a process for the manufacture of vinyl chloride wherein a mixture of 1,1-dichloroethane and 1,2-dichloroethane is employed as a feed material the improvement which comprises the step of contacting the mixture of 1,1-dichloroethane and 1,2-dichloroethane at a temperature between about 150 and 320 C. with a catalyst selected from the group consisting of metal halides and metal oxides, said metal being in group II of the periodic table and separately recovering vinyl chloride and 1,2- dichloroethane therefrom.

7 The process of claim 1 wherein the metal is magnesium.

8. The process of claim 1 wherein the metal is calcium.

9. The process of claim 1 wherein the metal is barium.

10, The process of claim 1 wherein the metal is zinc.

11. The process of claim 1 wherein the metal is cadmium.

References Cited in the file of this patent UNITED STATES PATENTS 2,134,102 Cass Oct. 25, 1938 2,183,036 Amos Dec. 12, 1939 2,410,541 Joyce Nov. 5, 1946 2,676,997 Brown et a1. Apr. 27, 1954 

1. A PROCESS FOR THE MANUFACTURE OF CHLOROETHYLENES WHICH COMPRISES CONTACTING A POLYCHLOROETHANE OF THE CLASS CONSISTING OF 1,1-DICHLOROETHANE AND 1,1,1-TRICHLOROETHANE AT A TEMPERATURE BETWEEN ABOUT 150* AND 500* C. WITH A CATALYST SELECTED FROM THE GROUP CONSISTING OFF METAL SALTS AND METAL OXIDES, SAID METAL BEING IN GROUP II OF THE PERIODIC TABLE. 